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Syllabus

[(a) 0.076 M/s (b) 0.038 M/s (c) 0.038 M/s]

^{-4}s^{-1},if the initial concentration of the reactant is 0.004 M ,what is the molarity after 20 minutes ?How long will it take for 25% of the reactant to react?_{2}---> 2a is first order in A_{2}.after 12.3 minutes 65% of A_{2}remains undecomposed . how long will it take to decompose 90% of A_{2}?what is the half life of the reaction?^{-1}to become 0.4 mol L^{-1}. how long will it take for the initial concentraation to become 0.3 mol L^{-1}_{a}) of the reaction (R = gas constant)(a) 1842.4 R (b) 921.2 R (c) 460.6 R (d) 230.3 R

54. In respect of the equation $K=A{e}^{-{E}_{a}/RT}$in chemical kinetics, which one of the following statement is correct

(a) 0.25 (b)0.5 (c)1 (d)2

please give the ans. as soon as possible.

5.27 A first order gas-phase reaction has an energy of activation of 240 kJ mol

^{-l}. If the frequenc factor of the reaction is calculate 1.6 x 10^{13}s^{-1}, Calculate its rate constant at 600 K. (2.056 x 10^{-8}s^{-1})reaction

ti+ +2ce4+ ti3+ +2ce3+ rate law for reaction

(a) 1/3 times (b) 2/3 times (c) 3 times (d) 6 times

why prepration of H2SO4 in contact process do not obey Raults law

Q.97. The activation energy for a reaction is 9.0 K cal/mol. The increase in the rate constant when its temperature is increased from 298 K to 308 K is

(a) 63 %

(b) 50 %

(c) 100 %

(d) 10 %

Q. What function of [X], plotted against time, will give a straight line for a second-order reaction?

(1) [X]

(2) $[X{]}^{2}$

(3) log [X]

(4) $\frac{1}{\left[X\right]}$

the integrated rate lawDERIVEfor Pseudo first order and second order reactions!! ASAP!!in detaileg:- 2FeCl

_{3}+SnCl_{2}=2FeCl +SnCl_{2}what if we are given thisreaction and asked to state whether it is a 1st/2nd/3rd ordered reaction and no information is given about its initial or final conc. also its rate is not given,then how to find?Q5.3 Consider the reaction 2A + 2B →2C + D. From the following data, calculate the order and rate constant of the reaction.

_{0}] / M_{0}] /M_{0}/Ma^{–1}0.244

0.244

0.160

0.320

0.06

0.12

For a first order reaction the time needed is 30min for the concentration to fall from 1.5M to 0.9M. The time needed for the fall in the concentration from 0.9M to 0.54M will beQ.5.25 The rate constant of a first order reaction at 25$\xb0$C is 0.24 ${s}^{-1}$. If the energy of activation of the reaction is 88 kJ $mo{l}^{-1}$, at what temperature would this reaction have rate constant of $4\times {10}^{-2}{s}^{-1}$?

(283.7 K)

Q5.2 Consider the reaction

$3\mathrm{I}\left(\mathrm{aq}\right)+{\mathrm{S}}_{2}{\mathrm{O}}_{8}^{2}\left(\mathrm{aq}\right)\to {\mathrm{I}}_{3}^{-}\left(\mathrm{aq}\right)+2{\mathrm{SO}}_{4}^{2-}\left(\mathrm{aq}\right)\phantom{\rule{0ex}{0ex}}\mathrm{At}\mathrm{a}\mathrm{particular}\mathrm{time}\mathrm{t},\frac{\mathrm{d}\left[{\mathrm{SO}}_{4}^{2-}\right]}{\mathrm{dt}}=2.2\times {10}^{-2}\mathrm{M}/\mathrm{s}.\phantom{\rule{0ex}{0ex}}\mathrm{What}\mathrm{are}\mathrm{the}\mathrm{value}\mathrm{of}\left(\mathrm{a}\right)-\frac{\mathrm{d}\left[{\mathrm{I}}^{-}\right]}{\mathrm{dt}}$

(b) $-\frac{\mathrm{d}\left[{\mathrm{S}}_{2}{\mathrm{O}}_{8}^{2-}\right]}{\mathrm{dt}}$ (c) $\frac{\mathrm{d}\left[{\mathrm{I}}_{3}^{-}\right]}{\mathrm{dt}}$ at the same time?

(a) 3.3 × 10

^{–2}M/s (b) 1.1 × 10^{–2}M/s(c) 1.1 × 10

^{–2}M/sAnswer me 1&2

(a) 273.15°C (b) O°C

(c) –373.15°C (D) –273.15°C

Q2. Na

_{2}CO_{3}_{ }is a salt of ______________.(a) strong acid and strong base

(b) strong acid and weak base

(c) weak acid and strong base

(d) weak acid and weak base

[(a) 0.076 M/s (b) 0.038 M/s (c) 0.038 M/s]